Given below are two statements :Statement I : | vedclass

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(D) The acidic strength of hydrides of group $16$ elements increases down the group due to the decrease in bond dissociation enthalpy. Thus,the order

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Statement $I$ is false but Statement $II$ is true.

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(D) The acidic strength of hydrides of group $16$ elements increases down the group due to the decrease in bond dissociation enthalpy. Thus,the order is $H_2Se The bond dissociation enthalpy decreases down the group as the bond length increases. Thus,$H_2Se$ has a higher bond dissociation enthalpy $(276 \ kJ/mol)$ compared to $H_2Te$ $(238 \ kJ/mol)$. Therefore,Statement $II$ is true.

Given below are two statements $:$
Statement $I : H_2Se$ is more acidic than $H_2Te$.
Statement $II : H_2Se$ has higher bond enthalpy for dissociation than $H_2Te$.
In the light of the above statements,choose the correct answer from the options given below.

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Given below are two statements $:$Statement $I : H_2Se$ is more acidic than $H_2Te$.Statement $II : H_2Se$ has higher bond enthalpy for dissociation than $H_2Te$.In the light of the above statements,choose the correct answer from the options given below.